Question: calculate pH of 50.0 mL acetate buffer + 1.00 mL 0.6 M NaOH Moles CH3COOH OH- CH3COO- before addition ? ? ? Addition ? ? ? after addition ? ? ? (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question: calculate pH of 50.0 mL acetate buffer + 1.00 mL 0.6 M NaOH
| Moles | CH3COOH | OH- | CH3COO- |
| before addition | ? | ? | ? |
| Addition | ? | ? | ? |
| after addition | ? | ? | ? |
(below is the data to answer the answer)
| Deionized water | Acetate Buffer | Ammonia Buffer | ||
| pH of solution | 6.62 | 4.59 | 9.49 | |
| Ph of solution after addition of 1 mL of 0.6 M NaOH | 12.41 | 4.71 | 9.50 | |
| pH of solution after addition of 1 mL of 0.6 M HCl | 1.38 | 3.87 | 9.24 | |
Preparation of Buffer solutions
Mass of sodium acetate in acetate buffer ~ 1.1981
Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81
Mass of ammonium chloride ~ 1.2721
Volume of 5.0 M NH4OH ~ 6.00
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